Question
Explain the oxidation states of Group $16$ elements.
✓
Answer
- Group $16$ elements have general electronic configuration, $ns^2 np^4,$
- They show variable oxidation states, $– 2, + 2, + 4$ and $-6.$
- Since all elements have $6$ valence electrons, they tend to gain or share $2$ electrons to complete an octet, and show common oxidation state $– 2.$
- Oxygen being highly electronegative, it shows the common oxidation state $-2$ in oxides $(H_2O, MgO).$ It shows $– 1$ oxidation state in peroxides $(H_2O_2, Na_2O_2)$ and $+ 2$ oxidation states in $OF_2.$
- Except oxygen all other elements have vacant d-orbitals, hence they show higher oxidation states $+ 4$ and $+ 6$. For example
- The stability of the $+ 6$ oxidation state decreases but the stability of the $+4$ oxidation state increases down the group due to the inert pair effect.
- Bonding in $+4$ and $+6$ oxidation states is covalent in nature.
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